Question

he reusable booster rockets of the U.S. space shuttle use a mixture of aluminum and ammonium perchlorate for fuel. A possible equation for this reaction is as follows. 3 Al(s) + 3 NH4ClO4(s) → Al2O3(s) + AlCl3(s) + 3 NO(g) + 6 H2O(g) What mass of Al should be used in the fuel mixture for every kilogram of NH4ClO4

Answer 1

Answer: 229.8 g of Al should be used in the fuel mixture for every kilogram of $NH_4ClO_4$

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}$

$\text{Number of moles of }NH_4ClO_4=\frac{1000g}{117.5g/mol}=8.510moles$

$3Al(s)+3NH_4ClO_4(s)\rightarrow Al_2O_3(s)+AlCl_3(s)+3NO(g)+6H_2O(g)$

According to stoichiometry:

3 moles of $NH_4ClO_4$ reacts with = 3 moles of aluminium

Thus 8.510 moles of $NH_4ClO_4$ react with = $\frac{3}{3}\times 8.510=8.510$ moles of aluminum

Mass of aluminium = $moles\times {molar mass}}=8.510mol\times 27g/mol=229.8g$